Classification of Elements and Periodicity in Properties
89686
EN of an atom is given by the average of EA and .....
1 $\mathrm{EN}$
2 Ionization energy
3 Electron affinity
4 Electropositive character
Explanation:
According to Mulliken, Electronegativity of an elements is the average of Ionization Potential and Electron affinity. Electronegativity $(\mathrm{EN})=\frac{\text { Ionization potential }+ \text { Electron affinity }}{2}$
A.P.EAMCET 1992
Classification of Elements and Periodicity in Properties
89687
Ionisation potential of $1 \mathrm{~s}$ electron is ..... than that of $2 \mathrm{~s}$ electron in the same atom.
1 Same
2 Lesser
3 Greater
4 None of these
Explanation:
Ionisation potential of 1 s electron is greater than that of $2 \mathrm{~s}$ electron in the same atom because former is more closer to the nucleus.
A.P.EAMCET 1992
Classification of Elements and Periodicity in Properties
89688
$\mathrm{Al}^{3+}$ ion has a lower ionic radius than $\mathrm{Mg}^{2+}$ ion because
1 $\mathrm{Mg}$ atom has less number of neutrons than $\mathrm{Al}$
2 $\mathrm{Al}^{3+}$ has a higher nuclear charge than $\mathrm{Mg}^{2+}$
3 their electronegativities are different
4 Al has a lower ionization potential than $\mathrm{Mg}$ atom
Explanation:
$\mathrm{Al}^{3+}$ ion has a lower ionic radius than $\mathrm{Mg}^{2+}$ ion because of $\mathrm{Al}^{3+}$ has a higher nuclear charge than $\mathrm{Mg}^{2+}$. Nuclear charge increase then ionic radius decrease.
A.P.EAMCET 1992
Classification of Elements and Periodicity in Properties
89689
Among the alkali metals, the metal with the highest ionisation potential is
1 $\mathrm{Na}$
2 $\mathrm{K}$
3 $\mathrm{Li}$
4 $\mathrm{Cs}$
Explanation:
Ionisation potential is decrease from down the group hence Li metal has highest ionisation potential.
Classification of Elements and Periodicity in Properties
89686
EN of an atom is given by the average of EA and .....
1 $\mathrm{EN}$
2 Ionization energy
3 Electron affinity
4 Electropositive character
Explanation:
According to Mulliken, Electronegativity of an elements is the average of Ionization Potential and Electron affinity. Electronegativity $(\mathrm{EN})=\frac{\text { Ionization potential }+ \text { Electron affinity }}{2}$
A.P.EAMCET 1992
Classification of Elements and Periodicity in Properties
89687
Ionisation potential of $1 \mathrm{~s}$ electron is ..... than that of $2 \mathrm{~s}$ electron in the same atom.
1 Same
2 Lesser
3 Greater
4 None of these
Explanation:
Ionisation potential of 1 s electron is greater than that of $2 \mathrm{~s}$ electron in the same atom because former is more closer to the nucleus.
A.P.EAMCET 1992
Classification of Elements and Periodicity in Properties
89688
$\mathrm{Al}^{3+}$ ion has a lower ionic radius than $\mathrm{Mg}^{2+}$ ion because
1 $\mathrm{Mg}$ atom has less number of neutrons than $\mathrm{Al}$
2 $\mathrm{Al}^{3+}$ has a higher nuclear charge than $\mathrm{Mg}^{2+}$
3 their electronegativities are different
4 Al has a lower ionization potential than $\mathrm{Mg}$ atom
Explanation:
$\mathrm{Al}^{3+}$ ion has a lower ionic radius than $\mathrm{Mg}^{2+}$ ion because of $\mathrm{Al}^{3+}$ has a higher nuclear charge than $\mathrm{Mg}^{2+}$. Nuclear charge increase then ionic radius decrease.
A.P.EAMCET 1992
Classification of Elements and Periodicity in Properties
89689
Among the alkali metals, the metal with the highest ionisation potential is
1 $\mathrm{Na}$
2 $\mathrm{K}$
3 $\mathrm{Li}$
4 $\mathrm{Cs}$
Explanation:
Ionisation potential is decrease from down the group hence Li metal has highest ionisation potential.
Classification of Elements and Periodicity in Properties
89686
EN of an atom is given by the average of EA and .....
1 $\mathrm{EN}$
2 Ionization energy
3 Electron affinity
4 Electropositive character
Explanation:
According to Mulliken, Electronegativity of an elements is the average of Ionization Potential and Electron affinity. Electronegativity $(\mathrm{EN})=\frac{\text { Ionization potential }+ \text { Electron affinity }}{2}$
A.P.EAMCET 1992
Classification of Elements and Periodicity in Properties
89687
Ionisation potential of $1 \mathrm{~s}$ electron is ..... than that of $2 \mathrm{~s}$ electron in the same atom.
1 Same
2 Lesser
3 Greater
4 None of these
Explanation:
Ionisation potential of 1 s electron is greater than that of $2 \mathrm{~s}$ electron in the same atom because former is more closer to the nucleus.
A.P.EAMCET 1992
Classification of Elements and Periodicity in Properties
89688
$\mathrm{Al}^{3+}$ ion has a lower ionic radius than $\mathrm{Mg}^{2+}$ ion because
1 $\mathrm{Mg}$ atom has less number of neutrons than $\mathrm{Al}$
2 $\mathrm{Al}^{3+}$ has a higher nuclear charge than $\mathrm{Mg}^{2+}$
3 their electronegativities are different
4 Al has a lower ionization potential than $\mathrm{Mg}$ atom
Explanation:
$\mathrm{Al}^{3+}$ ion has a lower ionic radius than $\mathrm{Mg}^{2+}$ ion because of $\mathrm{Al}^{3+}$ has a higher nuclear charge than $\mathrm{Mg}^{2+}$. Nuclear charge increase then ionic radius decrease.
A.P.EAMCET 1992
Classification of Elements and Periodicity in Properties
89689
Among the alkali metals, the metal with the highest ionisation potential is
1 $\mathrm{Na}$
2 $\mathrm{K}$
3 $\mathrm{Li}$
4 $\mathrm{Cs}$
Explanation:
Ionisation potential is decrease from down the group hence Li metal has highest ionisation potential.
Classification of Elements and Periodicity in Properties
89686
EN of an atom is given by the average of EA and .....
1 $\mathrm{EN}$
2 Ionization energy
3 Electron affinity
4 Electropositive character
Explanation:
According to Mulliken, Electronegativity of an elements is the average of Ionization Potential and Electron affinity. Electronegativity $(\mathrm{EN})=\frac{\text { Ionization potential }+ \text { Electron affinity }}{2}$
A.P.EAMCET 1992
Classification of Elements and Periodicity in Properties
89687
Ionisation potential of $1 \mathrm{~s}$ electron is ..... than that of $2 \mathrm{~s}$ electron in the same atom.
1 Same
2 Lesser
3 Greater
4 None of these
Explanation:
Ionisation potential of 1 s electron is greater than that of $2 \mathrm{~s}$ electron in the same atom because former is more closer to the nucleus.
A.P.EAMCET 1992
Classification of Elements and Periodicity in Properties
89688
$\mathrm{Al}^{3+}$ ion has a lower ionic radius than $\mathrm{Mg}^{2+}$ ion because
1 $\mathrm{Mg}$ atom has less number of neutrons than $\mathrm{Al}$
2 $\mathrm{Al}^{3+}$ has a higher nuclear charge than $\mathrm{Mg}^{2+}$
3 their electronegativities are different
4 Al has a lower ionization potential than $\mathrm{Mg}$ atom
Explanation:
$\mathrm{Al}^{3+}$ ion has a lower ionic radius than $\mathrm{Mg}^{2+}$ ion because of $\mathrm{Al}^{3+}$ has a higher nuclear charge than $\mathrm{Mg}^{2+}$. Nuclear charge increase then ionic radius decrease.
A.P.EAMCET 1992
Classification of Elements and Periodicity in Properties
89689
Among the alkali metals, the metal with the highest ionisation potential is
1 $\mathrm{Na}$
2 $\mathrm{K}$
3 $\mathrm{Li}$
4 $\mathrm{Cs}$
Explanation:
Ionisation potential is decrease from down the group hence Li metal has highest ionisation potential.
